Question

Consider the reaction: X + Y -> Z. FRom the data below, determine the Rate when [X] = 0.50M and [Y] = 0.25M.

Rate (M/s) [X](M) [Y](M)

0.053 ------0.10----0.50

0.127-------0.20----0.30

1.02---------0.40----0.60

0.254-------0.20----0.60

0.509-------0.40-----0.30

Answer #1

rate of the reaction -r =K[X]^{m} [Y]^{n}

m and n are orders with respect to X and Y. K is the rate constant

from experiment 2 , K[0.2]^{m}
[0.3]^{n}= 0.127 (1)

from experiment 4 K [0.2]^{m}
[0.6]^{n}= 0.254
(2)

Eq.2/ Eq.1 gives [2]^{n}= 2 n=1

experiment 3 K[0.4]^{m}
[0.6]^{n}= 1.02 (3)

Eq.3 / Eq.2 gives [2]^{m}= 1,02/0.254=4, m=2

The rate becomes -r = K[ X]^{2} [Y]^{1}

from experiment 1 0.053 =K[ 0.1]^{2}
[0.5]^{1}, K[ 0.005]

K= 0.053/0.005=10.6/M.s

The rare expression becomes -r =10.6 [X]^{2}
[Y]^{1}

at [X] =0.5M and Y= 0.25M rate= 10.6*[0.5]^{2}
[0.25]=0.6625 M/s

Consider the reaction X + Y → Z From the data in the table,
obtained at 360 K, (a) determine the overall order of the reaction
Initial Rate of Disappearance of X (M/s) [X] (M) [Y](M) 0.053 0.10
0.50 0.127 0.20 0.30 1.02 0.40 0.60 0.254 0.20 0.60 0.509 0.40 0.30
(b) determine the initial rate of disappearance of X when the
concentration of X is 0.50 M and that of Y is 0.30 M.

Consider the reaction X + Y → Z From the data in the table,
obtained at 360 K,
(a) determine the overall order of the reaction 2 Initial Rate
of Disappearance of X (M/s) [X] (M) [Y](M)
(b) determine the initial rate of disappearance of X when the
concentration of X is 0.40 M and that of Y is 0.20 M.
initial rate of disappearance of X
(m/s) [X]
(M)
[Y](M)
.053
.1
.5
.127
.2
.3
1.02
.4 ...

Consider the reaction and the initial concentration and initial
rate data below.
BrO3-(aq) + 5 Br- (aq) + 6 H+(aq) ® 3 Br2 (aq) + 3 H2O (l)
Experiment
[BrO3-], (M)
[Br-],(M)
[H+],(M)
Initial Rate (M/sec)
1
0.10
0.10
0.10
1.2 x 10-3
2
0.20
0.10
0.10
2.4 x 10-3
3
0.10
0.30
0.10
3.5 x 10-3
4
0.20
0.10
0.15
5.4 x 10-3
Determine the rate law for this reaction
What is the overall order of the rate law?...

Rate data for the reaction 2 CsF + XeF6 →
Cs2XeF8 were taken. Given the data below,
determine the rate law for the reaction.
Trial [CsF]0
(M)
[XeF6]0 (M)
rate0 (M/min)
1
0.10
0.20
0.0145
2
0.20
0.20
0.0289
3
0.30
0.40
0.0867

For the reaction A + B + C → products, the following
initial-rate data were obtained.
[A]0 (mol/L)
[B]0 (mol/L)
[C]0 (mol/L)
Initial Rate (mol/(L · s))
0.40
0.40
0.20
0.0160
0.20
0.40
0.40
0.0080
0.60
0.10
0.20
0.0015
0.20
0.10
0.20
0.0005
0.20
0.20
0.40
0.0020
What are the reaction orders with respect to A, B, and C,
respectively?
A.
0, 2, 1
B.
1, 1, 1
C.
1, 2, 0
D.
1, 2, 1
E.
0, 1, 1

Consider the following data showing the initial rate of a
reaction (A→products) at several different concentrations of A.
[A](M)
Initial Rate (M/s)
0.15
6.87×10−3
0.30
1.37×10−2
0.60
2.75×10−2
What is the rate law for this reaction?
Rate = k[A]3
Rate = k[A]
Rate = k
Rate = k[A]2
2.)
Consider the following data showing the initial rate of a
reaction (A→products) at several different concentrations of A.
[A](M)
Initial Rate (M/s)
0.15
2.75×10−2
0.30
2.75×10−2
0.60
2.75×10−2
What is the...

Consider the following data showing the initial rate of a reaction
at several different concentrations of A.
[A](M)
0.15
0.30
0.60
Initial Rate (M/s)
0.026
0.207
1.655
What is the order of the reaction? Express as an
integer.
What is the rate law?
Estimate the value of the rate constant, k.

For the reaction 2 A + B + 2C → 2 D + 3 E, we obtain the data in
the table below. What is this reaction's rate law (be sure to
calculate the value of k)? What is the reaction rate if each
reactant's concentration is 0.70 M. The temperature is
25oC.
[A]o
[B]o
[C]o
rate, vo (M s-1)
0.25
0.20
0.10
0.20
0.25
0.40
0.20
0.40
0.25
0.40
0.40
0.80
0.50
0.40
0.40
0.80
1.00
0.40
1.00
2.00...

determine the initial rate for a reaction that starts with 0.85
M of reagent A and 0.70 M of reagents B and C? Express your answer
to two significant figures and include the appropriate units.
Indicate the multiplication of units explicitly either with a
multiplication dot or a dash.
For the reaction A+B+C→D+E, the initial reaction rate was
measured for various initial concentrations of reactants. The
following data were collected:
Trial [A](M) [B](M) [C](M) Initial rate (M/s)
1 0.30 0.30...

Consider the gas-phase reaction between nitric oxide and bromine
at 273 ?C
2NO(g)+Br2(g)?2NOBr(g).
The following data for the initial rate of appearance of NOBr were
obtained:
Experiment
[NO](M)
[Br2](M)
Initial Rate of Appearance of NOBr(M/s)
1
0.10
0.20
24
2
0.25
0.20
150
3
0.10
0.50
60
4
0.35
0.50
735
rate=k[NO]2[Br2]
Calculate the average value of the rate constant for the
appearance of NOBr from the four data sets.
k= _______ M^-2s^-1
What is the rate of disappearance of...

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